Problem: AgCl would be least soluble at 25°C in ______ . 

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We’re being asked to determine in which solvent AgCl would be least soluble in.

The common ion effect states that the solubility of a salt is lower in the presence of a common ion. This means if there is a higher concentration of a common ion present, the less soluble a compound will be. The dissociation of AgCl in water is as follows:

The chloride ion, Cl, has a charge of –1. Silver then has a charge of +1:

AgCl(s)  Ag+(aq) + Cl(aq)

Among the given choices, only choices b, CaCl2, and c, HCl, contain a common ion, Cl. Pure water and 0.10 M HNO3 don't contain common ions so the solubility of AgCl is not lowered in those.

We’ll now determine which between 0.10 M CaCl2 and 0.10 M HCl has a higher Cl concentration: a higher Cl (common ion) concentration will lead to lower solubility of AgCl.

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AgCl would be least soluble at 25°C in ______ . 

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